AP Chemistry Final Exam 50 Multiple Choice questions, 60 ...

AP Chemistry Final Exam Version Q Fall 2006

50 Multiple Choice questions, 60 minutes

NO CALCULATORS MAY BE USED. You will have a periodic table.

Note: For all questions, assume that the temperature is 298 K, the pressure is 1.00 atmospheres, and solutions are aqueous unless otherwise specified.

Guessing: One-fourth of the number of questions you answer incorrectly will be subtracted from the number of questions you answer correctly.

You may write on this exam; however, you will only be given credit for answers recorded on the Scantron sheet.

NAME:

PERIOD: 1

2

3

4

December 12-14, 2006

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Version Q

Fall 06-07

Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select the option that best fits each statement. A choice may be used once, more than once, or not at all in each set.

Questions 1-3 A. Chlorine B. Helium C. Mercury D. Phosphorus

1. Solid at room temperature 2. Has a common oxidation state of +7 3. Colorless

Questions 4-6 A. Has covalent bond(s) B. Has ionic bond(s) C. Has unpaired electrons D. Has a positive electron affinity

4. CH4 5. NaH 6. Cr

Directions: Choose the best option for each question or statement.

7. A 5 L scuba tank sits in the sun, warming to 50 ?C with a pressure of 20 atm. What will be the pressure when the

temperature drops to 10 ?C when the tank is under water?

20 ? 50

A.

10

20 ? 10

5 ? 20 ? 283

B.

50 C.

323

20 ? 283 D. 5 323

20 ? 283 E. 323

8. How many oxygen atoms are present in one formula unit of cupric sulfate pentahydrate? A. 20 B. 13 C. 9 D. 5 E. 4

9. How many liters of oxygen measured at STP will be needed to completely react with 1 mole of H2S (g) in the following already balanced reaction? 2 H2S (g) + 3 O2 (g) 2 H2O (g) + 2 SO2 (g) A. 44.8 L B. 33.6 L C. 22.4 L D. 11.2 L E. 1.50 L

10. Which of the following is associated with an emission line in the Balmer series? A. Far-infrared B. Infrared C. Ultraviolet D. Visible E. X-ray

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11. Which series of elements represents increasing electronegativity? A. As, P, N B. Cl, S, P C. F, B, Li D. O, S, Se E. O, F, Ne

12. Which of the following is a nonpolar molecule? A. H2S B. NH3 C. SF4 D. SO2 E. SO3

13. What is the approximate molecular geometry of the central carbon in a molecule of propene? A. Bent B. Linear C. Tetrahedral D. Trigonal pyramidal E. Trigonal planar

14. The functional group in the molecule "CH3CHO" represents a/an: A. Alcohol B. Aldehyde C. Carboxylic acid D. Ether E. Ketone

15. How many milliliters of a 10-M solution of sulfuric acid should be added to distilled water to prepare a 1 L of a 1-M solution? A. 0.1 B. 1 C. 10 D. 100 E. 1000

16. How many hydrogen atoms are in 0.5 moles of hydrogen gas at STP? A. 0.5039 B. 1.0079 C. 3.011 x 1023 D. 6.022 x 1023 E. 1.204 x 1024

17. The name for V2O5 is: A. Divanadium pentoxide B. Vanadium oxide C. Vanadium (II) oxide (V) D. Vanadium (II) pentoxide E. Vanadium (V) oxide

18. What are the products when a solution of lead (II) nitrate is mixed with a solution of potassium chloride? A. PbCl2 (s) and KNO3 (aq) B. PbCl2 (aq) and KNO3 (aq) C. PbCl2 (s) and KNO3 (s) D. PbCl2 (aq) and KNO3 (s) E. PbK (s) and NO3Cl (s)

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19. Which of the following graphs best represents Boyle's law?

A.

B.

C.

D.

E.

V

V

V

V

P

P

T

1 / P

n

T

20. The empirical formula for a compound is CH2O. If the molar mass is approximately 90 g/mol, what is the molecular formula of the compound? A. CH2O B. C2H4O2 C. C3H6O3 D. C4H8O4 E. C6H12O6

21. Which arrangement of elements demonstrates the trend of increasing atomic radius? A. B, N, F B. I, Br, Cl C. Ge, P, O D. S, Al, Na E. H, He, Li

22. Which of the following atoms or ions are paramagnetic?

I.

Ar

II. P

III. Zn2+

A. I only B. II only C. III only D. I and II E. I and III

23. A sample of barium chloride dihydrate is heated. Which error would cause the experimental number of moles of water determined to be higher than the actual amount of moles of water? A. All of the water is not driven (by heating) from the hydrate. B. An inert, anhydrous impurity was in the hydrated sample. C. Some of the hydrate is lost due to splattering out of the crucible. D. The hydrated sample is not heated to a constant mass. E. The flame color is yellow-orange.

24. The following compounds are correctly matched to the statement at right EXCEPT:

Compound A. Ba(C2H3O2)2 B. Cu(NO3)2 C. Na2Cr2O7 D. KCl E. LiBr

Statement flame test is green solution is blue solution is orange solution is lilac flame test is red

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25. Which of the following will result in the production of H2 (g)?

I.

Magnesium is added to a hydrochloric acid.

II. Silver nitrate is added to sodium hydroxide.

III. Sodium is added to water.

A. I only

B. II only

C. III only

D. I and II only

E. I and III only

26. A student performs an experiment that involves burning a metal to form its oxide, and records the following data:

Mass of weighing paper only

1.120 g

Mass of weighing paper and metal

1.170 g

Mass of weighing paper and metal oxide 1.20 g

How many significant figures should be used to report the mass ratio of oxygen to metal in the final product? A. 1 B. 2 C. 3 D. 4 E. 5

27. Addition of which of the following solutions will allow you to differentiate between solutions of AgNO3 and Ag2SO4? A. KCl B. NH4NO3 C. Na2CO3 D. Ba(NO3)2 E. Zn(C2H3O2)2

28. What is the concentration of sodium ion when 500 mL of 0.5 M NaNO3 is mixed with 1000 mL of 0.25 M Na2CrO4 solution? A. 0.25 M B. 0.5 M C. 0.75 M D. 1 M E. 1.25 M

29. Use the data below to determine the enthalpy change of the following already balanced reaction: 2 WO3 (s) + 6 H2 (g) 2 W (s) + 6 H2O (g)

Data: 2 W (s) + 3 O2 (g) 2 WO3 (s) 2 H2 (g) + O2 (g) 2 H2O (g)

H = -1750 kJ H = -500 kJ

A. -3250 kJ B. -2250 kJ C. -1000 kJ D. 250 kJ E. 2250 kJ

30. Which gas deviates the most from the behavior of an ideal gas at STP? A. Ar B. CO C. I2 D. O2 E. CH4

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